Recall that the freezing point of a solution is lower than that of the pure solvent and the change in freezing point (ΔTf) is given by:
The change in freezing point is also related to the molality of the solution:
where:
i = van’t Hoff factor
m = molality of the solution (in m or mol/kg)
Kf = freezing point depression constant (in ˚C/m)
Recall that the molality of a solution is given by:
Solute | Expected | Measured |
Nonelectrolyte | 1 | 1 |
NaCl | 2 | 1.9 |
MgSO4 | 2 | 1.3 |
MgCl2 | 3 | 2.7 |
K2SO4 | 3 | 2.6 |
FeCl3 | 4 | 3.4 |
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